Chlorine Atom and Lewis Structures

The video tutorial explains how to draw the Lewis structure for the CL3- ion. It begins by calculating the total valence electrons, considering the negative charge. The tutorial then demonstrates placing electrons between chlorine atoms to form bonds and complete octets. It addresses the issue of extra electrons by expanding the octet on the central chlorine atom. Finally, it discusses the formal charges, ensuring the structure reflects the negative ion correctly.

How many total valence electrons are present in the Cl3- ion?

• 20

• 21

• 22

• 23

What is the significance of the negative charge in Cl3-?

• It indicates a missing electron

• It shows an extra proton

• It represents an additional electron

• It means the molecule is neutral

What is the first step in arranging the chlorine atoms for the Cl3- Lewis structure?

• Create a circle

• Form a square

• Arrange them in a line

• Place them in a triangle

After forming initial bonds, how many valence electrons are left unused?

• 0

• 1

• 2

• 3

What allows the central chlorine atom to hold more than eight electrons?

• It is a noble gas

• It has an expanded octet

• It is positively charged

• It is a metal

Where are the leftover electrons placed in the Cl3- Lewis structure?

• On the outer chlorines

• They are removed

• On the central chlorine

• In a separate orbital

How does the expanded octet affect the central chlorine atom?

• It reduces its size

• It makes it unstable

• It allows more than eight electrons

• It changes its color

What is the formal charge on the central chlorine atom in Cl3-?

• -2

• -1

• 0

• +1

Why is the formal charge important in determining the best Lewis structure?

• It helps in identifying the number of bonds

• It ensures the structure is stable

• It determines the color of the compound

• It affects the boiling point

What is the final step in verifying the Cl3- Lewis structure?

• Checking the color

• Validating the formal charges

• Calculating the molecular weight

• Measuring the bond length